Acids and Bases: Buffer Solutions 1

Having talked about weak acids and bases, not it's time for buffers. Prof Al, form AUT's chemistry department, outlines the fundamentals of buffer solutions, and shows how to get and equation named after yourself for merely rearranging another question. The worked problems: 1) 1.00 L of a buffer solution was prepared in which [CH₃COOH] = 0.150 mol L⁻¹ and [CH₃COO⁻] = 0.225 mol L⁻¹. Calculate the pH of this buffer solution, given that pKa(CH₃COOH) = 4.74. 2) If f 100 mL of 0.200 mol L⁻¹ HCl is added to the above buffer solution.